Consider the equation:
CHCl3(g)+Cl2(g) > CCl4(g)+HCl(g)
The initial rate of the reaction is measured at several different concentrations of the reactants with the following results: [CHCl3](M) [Cl2](M) Initial rate (M/s)
0.010 0.010 0.0035
0.020 0.010 0.0069
0.020 0.020 0.0098
0.040 0.040 0.027
1. From the data, choose the correct rate law for the reaction.
Rate = k[CHCl3][Cl2]^2Rate = k[CHCl3]^2[Cl2]^1/2Rate = k[CHCl3][Cl2]Rate = k[CHCl3][Cl2]^1/2
2. the rate constant (k) for the reaction. Express your answer using three significant figures.

1.

2. The rate constant (k) for the reaction is

Explanation:

Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.

k= rate constant

x = order with respect to

y = order with respect to

n = x+y= Total order

1. a) From trial 1:  (1)

From trial 2:   (2)

Dividing 2 by 1 :

therefore x=1.

b)  From trial 2:   (3)

From trial 3:   (4)

Dividing 4 by 3:

therefore

2. to find rate constant using trial 1:

c. 75.7

i think that is the right